2H 2 S (g) = 2H 2 (g) + S 2 (g) When heated hydrogen sulfide gas decomposes acco

Question

2H2S (g) = 2H2 (g) + S2 (g)

When heated hydrogen sulfide gas decomposes according to the equation above. A 3.40g smple of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72 x10-2 mol of S2 (g) is present at equilibrium.

a) Write the expression for the equilibrium constant, Kc for the decomposition reaction represented above.

b) Calculate the equilibrium concentration in M of H2 (g) and H2S (g) in the container 483 K

c) Calculate the value of the equilibrium constant Kc for the decomposition reaction of 483K

Explanation / Answer

K =[ H2 ]^2 [S2 ] / [H2S ] ^2

2H2S (g) = 2H2 (g) + S2 (g)

When heated hydrogen sulfide gas decomposes according to the equation above. A 3.40g smple of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72 x10-2 mol of S2 (g) is present at equilibrium.

a)      Write the expression for the equilibrium constant, Kc for the decomposition reaction represented above

K =[ H2]^2 [S2] / [H2S ] ^2

b) Calculate the equilibrium concentration in M of H2 (g) and H2S (g) in the container 483 K

H2S

2H2

S2

I

0

0

C

-5.95 X10^-2

5.95 X10^-2

2.98X10^-2

E

2.03 X10^-2

5.95 X10^-2

2.98X10^-2

M of H2 (g)-------------- 5.95 X10^-2

and H2S (g)------------------ 2.03 X10^-2

in the

c) Calculate the value of the equilibrium constant Kc for the decomposition reaction of 483K

K =[ 5.95 X10^-2]^2 [2.98X10^-2] / [2.03 X10^-2 ] ^2 = 0.256

H2S

2H2

S2

I

0

0

C

-5.95 X10^-2

5.95 X10^-2

2.98X10^-2

E

2.03 X10^-2

5.95 X10^-2

2.98X10^-2

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